1 - Periodic Table

Question 1

Relative Isotopic Mass?

Answer 1

Is the mass of an isotope, relative to 1/12 of the mass of an atom of carbon -12

Question 2

Relative atomic mass?

Answer 2

Is the weighted mean mass of an atom of an element, relative to 1/12 of the mass of an atom of carbon 12

Question 3

How is an ion formed?

Answer 3

By the loss or gaining of electrons

Question 4

Relative charge of a proton?

Answer 4

+1

Question 5

Relative charge of a neutron?

Answer 5

0

Question 6

Relative charge of an electron?

Answer 6

-1

Question 7

What is the mass number?

Answer 7

The biggest number, contains protons and neutrons

Question 8

What is the proton number?

Answer 8

number of protons + electrons

Question 9

Calculating relative atomic mass

Answer 9

75. 78 % of chlorine -35
76. 22% of chlorine -37

75.78 x 35 + 24.22 x 37 / 100

Question 10

Calculating moles?

Answer 10

How many moles of phosphorus pentoxide (P4O10) are in 85.2g?
P= 31
O=16
31x4 +16x10 = 284

85.2 / 284 = 0.3 moles

Question 11

Relative molecular mass?

Answer 11

N2 = 14 x 2 = 28

Question 12

Relative atomic mass?

Answer 12

Copper: 120.8% = 63
54% = 65

120.8 x 63 + 54 x 65/ 174.8
= 63.6

Question 13

Stages of mass spectrometry?

Answer 13

Gas injected in ionizer with electrons.
Beam of electrons is bombarded at electrons and sample is ionized.
Ions are accelerated in an electric field.
Then bend through magnetic field.
Deflected by electric field.

Question 14

What is the vacuum for in a mass spectrometer?

Answer 14

Means there’s no interference from other ions.

High energy electrons are used to make the positive ion

Question 15

Flame test: sodium chloride?

Answer 15

Yellow/ orange

Question 16

Flame test: Lithium chloride?

Answer 16

red/ pink

Question 17

Flame test: Calcium chloride?

Answer 17

yellow/ orange

Question 18

Flame test: Barium chloride?

Answer 18

green

Question 19

Flame test: Copper chloride?

Answer 19

Green/blue

Question 20

Flame test: Potassium chloride?

Answer 20

lilac/ pink

Question 21

Emission spectra?

Answer 21

If an electron takes in energy from its surroundings it’s excited to a higher energy level. When they drop to a lower energy level, they release this energy. (this is what we observe)

Question 22

how many electrons does the S orbital hold?

Answer 22

2 electrons

Question 23

How many electrons does the P orbital hold?

Answer 23

6 electrons

Question 24

How many electrons does the D orbital hold?

Answer 24

10 electrons

Question 25

How many electrons does the F orbital hold?

Answer 25

14 electrons

Question 26

First 7 electronic configuration?

Answer 26

1s2s2p3s3p4s3d

Question 27

Electronic configuration of Argon? 18 electrons

Answer 27

1s2, 2s2, 2p6, 3s2, 3p6

Question 28

Using the noble gas in the above row to shorten electronic configuration

Answer 28

Scandium 21 Argon = 18

(Ar) 3s2, 3p1

Question 29

Hunds rule?

Answer 29

Electrons will occupy the orbitals singularly before pairing takes place.

Question 30

Pauli’s exclusion principle?

Answer 30

2 electrons cannot occupy the same orbital, unless they have opposite spins.

Question 31

Chromuim and copper exceptions?

Answer 31

Both their 3d orbitals fill before their 4s orbitals

Question 32

Which shell empties first when forming ions, 3d or 4s?

Answer 32

4s, because it takes less energy.

Question 33

First ionisation energies?

Answer 33

Is the energy needed to remove 1 electron from each atom, in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

Question 34

First Ionisation energies?

Answer 34

Generally INCREASE across a period

DECREASE down a group

Question 35

First ionisation energies, exceptions?

Answer 35

groups 2+3 and 5+6

Question 36

Atomic radius? (distance from the nucleus)

Answer 36

The more shells an atom has, and therefore the further away the outer electrons are from the nucleus, the less attraction they experience!

Question 37

Nuclear charge?

Answer 37

The more protons, the greater the nuclear charge, the greater the attraction they experience!

Question 38

Electron shielding

Answer 38

As the number of electrons between outer electrons and the nucleus increases, the outer electrons feel less attraction towards the nuclear charge (shielding)

Question 39

First ionisation energy of chlorine?

Answer 39

Cl (g) — Cl+ (g) + e-

Question 40

Second Ionisation energies?

Answer 40

Each ionisation energy is greater than the last!

Shells are drawn slightly closer to the nucleus when electrons are removed, because there is less repulsion.

Question 41

Successive ionisation energies?

Answer 41

As you remove electrons, you’re pulling against the positive nucleus, therefore there is less repulsion between the electrons and each shell will be drawn slightly closer to the nucleus.

Question 42

Successive ionisation energies on graphs?

Answer 42

The rise indicates the jump to the next quantum shell.

Question 43

Periodicity?

Answer 43

studying of the trends as we go across the periodic table

Question 44

Atomic radius DECREASES across a period.

Answer 44

because the increase in protons and electrons fills more shells, and therefore shielding increases

Question 45

NUCLEAR CHARGE INCREASES across the periodic table

Answer 45

because the number of protons in the nucleus increases

Question 46

Period 3

Answer 46

ATOMIC radius increases as you go down the table